Question 1

What mass (g)of barium iodide is contained in 188 mL of a barium iodide solution that has an iodide ion concentration of 0.532 M?

Accepted Answer

A) 19.6 
B) 39.1 
C) 19,600 
D) 39,100 
E) 276 
A) 19.6 
B) 39.1 
C) 19,600 
D) 39,100 
E) 276

Question 2

Which solution has the same number of moles of KCl as 75.00 mL of 0.250 M solution of KCl?

Accepted Answer

A) 20.0 mL of 0.200 M solution of KCl 
B) 25.0 mL of 0.175 M solution of KCl 
C) 129 mL of 0.145 M solution of KCl 
D) 50.0 mL of 0.125 M solution of KCl 
E) 100 mL of 0.0500 M solution of KCl 
A) 20.0 mL of 0.200 M solution of KCl 
B) 25.0 mL of 0.175 M solution of KCl 
C) 129 mL of 0.145 M solution of KCl 
D) 50.0 mL of 0.125 M solution of KCl 
E) 100 mL of 0.0500 M solution of KCl

Question 3

Calculate the number of grams of solute in 500.0 mL of 0.159 M KOH.

Accepted Answer

A) 176 
B) 1.42 
C) 4.46 × 103 
D) 4.46 
E) 1.42 × 10-3 
A) 176 
B) 1.42 
C) 4.46 × 103 
D) 4.46 
E) 1.42 × 10-3

Question 4

The molarity of a solution prepared by diluting 43.72 mL of 1.005 M aqueous K2Cr2O7 to 500. mL is ________.

Accepted Answer

A) 0.0879 
B) 87.9 
C) 0.0218 
D) 0.0115 
E) 0.870 
A) 0.0879 
B) 87.9 
C) 0.0218 
D) 0.0115 
E) 0.870

Question 5

Which of the following are weak electrolytes? HNO3
HF
NH3
LiBr

Accepted Answer

A) HNO3, LiBr 
B) HNO3, HF, NH3, LiBr 
C) HF, LiBr 
D) HF, NH3 
E) HNO3, NH3, LiBr 
A) HNO3, LiBr 
B) HNO3, HF, NH3, LiBr 
C) HF, LiBr 
D) HF, NH3 
E) HNO3, NH3, LiBr

Question 6

Of the species below, only ________ is not an electrolyte.

Accepted Answer

A) HBr 
B) LiCl 
C) Ne 
D) KOH 
E) NaNO3 
A) HBr 
B) LiCl 
C) Ne 
D) KOH 
E) NaNO3

Question 7

Which one of the following is a diprotic acid?

Accepted Answer

A) nitric acid 
B) chloric acid 
C) phosphoric acid 
D) hydrofluoric acid 
E) sulfuric acid 
A) nitric acid 
B) chloric acid 
C) phosphoric acid 
D) hydrofluoric acid 
E) sulfuric acid

Question 8

What is the molarity of a NaOH solution if 15.5 mL of a 0.220 M H2SO4 solution is required to neutralize a 25.0-mL sample of the NaOH solution?

Accepted Answer

A) 0.273 
B) 0.355 
C) 0.710 
D) 42.6 
E) 0.136 
A) 0.273 
B) 0.355 
C) 0.710 
D) 42.6 
E) 0.136

Question 9

When aqueous solutions of ________ are mixed, a precipitate forms.

Accepted Answer

A) NiBr2 and AgNO3 
B) NaI and KBr 
C) K2SO4 and CrCl3 
D) KOH and Ba(NO3)2 
E) Li2CO3 and CsI 
A) NiBr2 and AgNO3 
B) NaI and KBr 
C) K2SO4 and CrCl3 
D) KOH and Ba(NO3)2 
E) Li2CO3 and CsI

Question 10

A 31.5 mL aliquot of HNO3 (aq)of unknown concentration was titrated with 0.0134 M NaOH (aq). It took 23.9 mL of the base to reach the endpoint of the titration. The concentration (M)of the acid was ________.

Accepted Answer

A) 0.0102 
B) 0.0051 
C) 0.0204 
D) 0.227 
E) 1.02 
A) 0.0102 
B) 0.0051 
C) 0.0204 
D) 0.227 
E) 1.02

Question 11

One method for removal of metal ions from a solution is to convert the metal to its elemental form so it can be filtered out as a solid. Which metal can be used to remove aluminum ions from solution?

Accepted Answer

A) zinc 
B) cobalt 
C) lead 
D) copper 
E) none of these 
A) zinc 
B) cobalt 
C) lead 
D) copper 
E) none of these

Question 12

Which of the following would require the largest volume of 0.100 M sodium hydroxide solution for neutralization?

Accepted Answer

A) 10.0 mL of 0.0500 M phosphoric acid 
B) 20.0 mL of 0.0500 M nitric acid 
C) 5.0 mL of 0.0100 M sulfuric acid 
D) 15.0 mL of 0.0500 M hydrobromic acid 
E) 10.0 mL of 0.0500 M perchloric acid 
A) 10.0 mL of 0.0500 M phosphoric acid 
B) 20.0 mL of 0.0500 M nitric acid 
C) 5.0 mL of 0.0100 M sulfuric acid 
D) 15.0 mL of 0.0500 M hydrobromic acid 
E) 10.0 mL of 0.0500 M perchloric acid

Question 13

How many moles of Co2+ are present in 0.200 L of a 0.400 M solution of CoI2?

Accepted Answer

A) 2.00 
B) 0.500 
C) 0.160 
D) 0.0800 
E) 0.0400 
A) 2.00 
B) 0.500 
C) 0.160 
D) 0.0800 
E) 0.0400

Question 14

What is the concentration (M)of CH3OH in a solution prepared by dissolving 10.2 g of CH3OH in sufficient water to give exactly 230 mL of solution?

Accepted Answer

Question 15

Which ions are spectator ions in the formation of a precipitate of AgCl via combining aqueous solutions of CoCl2 and AgNO3?

Accepted Answer

A) Co2+ and NO3- 
B) NO3- and Cl- 
C) Co2+ and Ag+ 
D) Cl- 
E) NO3- 
A) Co2+ and NO3- 
B) NO3- and Cl- 
C) Co2+ and Ag+ 
D) Cl- 
E) NO3-

Question 16

Which of the following are strong acids? HI
HNO3
HF
HBr

Accepted Answer

A) HF, HBr 
B) HI, HNO3, HF, HBr 
C) HI, HF, HBr 
D) HNO3, HF, HBr 
E) HI, HNO3, HBr 
A) HF, HBr 
B) HI, HNO3, HF, HBr 
C) HI, HF, HBr 
D) HNO3, HF, HBr 
E) HI, HNO3, HBr

Question 17

A solution is prepared by mixing 15.0 mL of 0.100 M HCl and 5.00 mL of 0.200 M NaCl. What is the molarity of chloride ion in this solution?

Accepted Answer

A) 0.175 
B) 8.00 
C) 1.25 
D) 0.0250 
E) 0.125 
A) 0.175 
B) 8.00 
C) 1.25 
D) 0.0250 
E) 0.125

Question 18

In which reaction does the oxidation number of oxygen increase?

Accepted Answer

A) Ba(NO3)2 (aq) + K2SO4 (aq) → BaSO4 (s) + 2KNO3 (aq) 
B) HCl (aq) + NaOH (aq) → NaCl (aq) + H2O (l) 
C) MgO (s) + H2O (l) → Mg(OH)2 (s) 
D) 2SO2 (g) + O2 (g) → 2SO3 (g) 
E) 2H2O (l) → 2H2 (g) + O2 (g) 
A) Ba(NO3)2 (aq) + K2SO4 (aq) → BaSO4 (s) + 2KNO3 (aq) 
B) HCl (aq) + NaOH (aq) → NaCl (aq) + H2O (l) 
C) MgO (s) + H2O (l) → Mg(OH)2 (s) 
D) 2SO2 (g) + O2 (g) → 2SO3 (g) 
E) 2H2O (l) → 2H2 (g) + O2 (g)

Question 19

How many milliliters of a stock solution of 11.7 M HNO3 would be needed to prepare 0.500 L of 0.500 M HNO3?

Accepted Answer

A) 0.0468 
B) 21.4 
C) 2.93 
D) 46.8 
E) 0.0214 
A) 0.0468 
B) 21.4 
C) 2.93 
D) 46.8 
E) 0.0214

Question 20

In the following reaction, which species is reduced? Au(s) + 3NO3-(aq) + 6H+(aq) → Au3+(aq) + NO(g) + 3H2O (l)
H+
N+5
O2-
H2O
Au

Accepted Answer

A) H+ 
B) N+5 
C) O2- 
D) H2O 
E) Au 
A) H+ 
B) N+5 
C) O2- 
D) H2O 
E) Au

Exam 4: Aqueous Reactions and Solution Stoichiometry

What mass (g)of barium iodide is contained in 188 mL of a barium iodide solution that has an iodide ion concentration of 0.532 M?

Which solution has the same number of moles of KCl as 75.00 mL of 0.250 M solution of KCl?

Calculate the number of grams of solute in 500.0 mL of 0.159 M KOH.

The molarity of a solution prepared by diluting 43.72 mL of 1.005 M aqueous K2Cr2O7 to 500. mL is ________.

Which of the following are weak electrolytes? HNO3 HF NH3 LiBr

Of the species below, only ________ is not an electrolyte.

Which one of the following is a diprotic acid?

What is the molarity of a NaOH solution if 15.5 mL of a 0.220 M H2SO4 solution is required to neutralize a 25.0-mL sample of the NaOH solution?

When aqueous solutions of ________ are mixed, a precipitate forms.

A 31.5 mL aliquot of HNO3 (aq)of unknown concentration was titrated with 0.0134 M NaOH (aq). It took 23.9 mL of the base to reach the endpoint of the titration. The concentration (M)of the acid was ________.

One method for removal of metal ions from a solution is to convert the metal to its elemental form so it can be filtered out as a solid. Which metal can be used to remove aluminum ions from solution?

Which of the following would require the largest volume of 0.100 M sodium hydroxide solution for neutralization?

How many moles of Co2+ are present in 0.200 L of a 0.400 M solution of CoI2?

What is the concentration (M)of CH3OH in a solution prepared by dissolving 10.2 g of CH3OH in sufficient water to give exactly 230 mL of solution?

Which ions are spectator ions in the formation of a precipitate of AgCl via combining aqueous solutions of CoCl2 and AgNO3?

Which of the following are strong acids? HI HNO3 HF HBr

A solution is prepared by mixing 15.0 mL of 0.100 M HCl and 5.00 mL of 0.200 M NaCl. What is the molarity of chloride ion in this solution?

In which reaction does the oxidation number of oxygen increase?

How many milliliters of a stock solution of 11.7 M HNO3 would be needed to prepare 0.500 L of 0.500 M HNO3?

In the following reaction, which species is reduced? Au(s) + 3NO3-(aq) + 6H+(aq) → Au3+(aq) + NO(g) + 3H2O (l) H+ N+5 O2- H2O Au

Introduction: Matter and Measurement

Atoms, Molecules, and Ions

Stoichiometry: Calculations With Chemical Formulas and Equations

Thermochemistry

Electronic Structure of Atoms

Periodic Properties of the Elements

Basic Concepts of Chemical Bonding

Molecular Geometry and Bonding Theories

Gases

Liquids and Intermolecular Forces

Solids and Modern Materials

Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acid-Base Equilibria

Additional Aspects of Aqueous Equilibria

Chemistry of the Environment

Chemical Thermodynamics

Electrochemistry

Nuclear Chemistry

Chemistry of the Nonmetals

Transition Metals and Coordination Chemistry

The Chemistry of Life: Organic and Biological Chemistry

Filters

The molarity of a solution prepared by diluting 43.72 mL of 1.005 M aqueous K₂Cr₂O₇ to 500. mL is ________.

Which of the following are weak electrolytes? HNO₃ HF NH₃ LiBr

What is the molarity of a NaOH solution if 15.5 mL of a 0.220 M H₂SO₄solution is required to neutralize a 25.0-mL sample of the NaOH solution?

A 31.5 mL aliquot of HNO₃ (aq)of unknown concentration was titrated with 0.0134 M NaOH (aq). It took 23.9 mL of the base to reach the endpoint of the titration. The concentration (M)of the acid was ________.

How many moles of Co²⁺ are present in 0.200 L of a 0.400 M solution of CoI₂?

What is the concentration (M)of CH₃OH in a solution prepared by dissolving 10.2 g of CH₃OH in sufficient water to give exactly 230 mL of solution?

Which ions are spectator ions in the formation of a precipitate of AgCl via combining aqueous solutions of CoCl₂ and AgNO₃?

Which of the following are strong acids? HI HNO₃ HF HBr

How many milliliters of a stock solution of 11.7 M HNO₃ would be needed to prepare 0.500 L of 0.500 M HNO₃?

In the following reaction, which species is reduced? Au(s) + 3NO₃^-(aq) + 6H⁺(aq) → Au³⁺(aq) + NO(g) + 3H₂O (l) H⁺ N⁺⁵ O^2- H₂O Au